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Chemistry IGCSE > Unit 11 - Organic chemistry > Flashcards

Unit 11 - Organic chemistry Flashcards

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1
Q

Homologous series

A

A family of compounds that will have the same general formula and similar chemical properties

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2
Q

4 Homologous series

A
  • Alkanes
  • Alkenes
  • Alcohols
  • Carboxylic acids
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2
Q

Functional group

A

An atom or group of atoms that determines the chemical properties of the compound

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3
Q

General formula for alkanes

A

C(n)H(2n+2)

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4
Q

General formula for alkenes

A

C(n)H(2n)

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5
Q

General formula for alcohols

A

C(n)H(2n+1)OH

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6
Q

General formula for carboxylic acids

A

C(n)H(2n+1)COOH

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7
Q

Saturated compounds

A

All single bonds for carbon = C-C

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8
Q

Unsaturated compound

A

One or more are not single bonds for carbon

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9
Q

Trend with longer CH chains in structural formulas

A

Stronger intermolecular forces

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10
Q

Structural isomers

A

Compounds with the same molecular formula but different structural formulae

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11
Q

Suffix for alkanes

A
  • ane
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12
Q

Suffix for alkenes

A
  • ene
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13
Q

Suffix for alcohols

A
  • ol
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14
Q

Suffix for carboxylic acids

A
  • oic acid
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15
Q

Molecular formula for methane

A
  • CH4
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16
Q

Molecular formula for ethane

A
  • C2H6
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17
Q

Ethene formula

A

C2H4

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18
Q

Ethanol formula

A

C2H5OH

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19
Q

Ethanoic acid formula

A

CH3COOH

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20
Q

Product of alkanes reacting with chlorine

A

Chloroalkanes

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21
Q

Chloromethane composition

A

CH3Cl

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22
Q

Product of alkenes reacting with bromine

A

Dibromoalkanes

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23
Q
A
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24
Q

Product of alcohols reacting with carboxylic acids

A

Esters and water

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25
Q

4 common prefixes & number of carbon atoms

A
  • Meth - 1
  • Eth - 2
  • Prop - 3
  • But - 4
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26
Q

Fuel

A

A chemical substance that when reacted releases energy

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27
Q

3 main fuels

A
  • Coal
  • Natural gas
  • Petroleum - crude oil & hydrocarbon products
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28
Q

Equation for natural gas reaction

A

Methane + Oxygen –> Carbon dioxide + water

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29
Q

Petroleum composition

A
  • Mixture of Hydrocarbons
  • 30% alkanes
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30
Q

Different impurities in petroleum & their boiling points & uses

A
  • Refinery gas - <40˚C - Bottled gas
  • Petrol - 40-205˚C - Petrol/gas
  • Naphtha - 60-100˚C - Chemical feedstock
  • Kerosene - 175-325˚C - jet fuel, paraffin for lighting & heating
  • Diesel - 250-350˚C - Diesel fuels
  • Lubricating oil - 300-370˚C - Lubricating oils, waxes & polishes
  • Fuel oil - 370-600˚C - Fuel for ships. factories and central heating
  • Bitumen - >600˚C - Bitumen for roads and roofing
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31
Q

Viscosity

A

The property of a material describing its resistance to flow as a liquid

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32
Q
A
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32
Q
A
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33
Q

Correlation with carbon atoms and boiling point

A
  • More carbon atoms leads to having a higher boiling point
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34
Q

Method of separation for petroleum

A

Fractional distillation

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35
Q

Correlation with height of fractional tower and boiling point

A
  • Liquids with lower boiling points are at the top
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36
Q

Correlation with viscosity and number of carbon atoms

A
  • More carbon atoms leads to higher viscosity
37
Q

Correlation with volatility and number of carbon atoms

A
  • More carbon atoms leads to less volatility
38
Q

Number of carbon atoms per fraction of petroleum

A
  • Gasoline - 5-6
  • Kerosene - 10-15
  • Lubricating oil - 25-40
  • Bitumen - 40+
39
Q

Bonds in alkanes

A
  • Single covalent bonds
  • Saturated
  • Strong covalent bonds
40
Q
A
41
Q

Physical properties of first six alkanes (#Carbon atoms, boiling point, state at room temp.)

A
  • Methane - 1 - -161˚C - gas
  • Ethane - 2 - -89˚C - gas
  • Propane - 3 - -42˚C - gas
  • Butane - 4 - -1˚C - gas
  • Pentane - 5 - 36˚C - liquid
  • Hexane - 6 - 69˚C - liquid
42
Q

Reaction that needs to happen for alkanes to be used as a fuel

A
  • Combustion - exothermic reaction
  • Incomplete combustion - leads to carbon monoxide gas
43
Q

Substitution reactions with alkanes

A

When alkanes react with chlorine, a hydrogen atom is replaced with a chlorine atom to make chloroalkanes - UV is needed for activation energy

44
Q

Substitution reaction

A

An atom or group of atoms in a molecule is replaced by a different atom or group of atoms

45
Q

Photochemical reactions

A

Reactions that need light energy

46
Q

Cracking

A

Chemical process that breaks down larger alkane molecules to produce smaller alkane molecules and alkene molecules and hydrogen

47
Q

Reason for cracking

A
  • Get fuels from large alkane molecules
  • Produce alkenes which are used to make polymers/plastics
48
Q

Conditions needed for cracking

A
  • Heating (500˚C)
  • Catalyst
49
Q
A
50
Q

Bonding in alkenes

A
  • Double C=C bond and absence of two hydrogens
  • Double bonds can be broken to form single bonds and allow other atoms to be added
  • Unsaturated compounds
51
Q

Correlation with bonding and distance of nuclei

A

-More bonds/sharing more electrons drawn nuclei closer

52
Q

Chemical test for unsaturated double bonds in alkenes

A
  • Test with Bromine water
  • If water changes from brown to colorless, a double bond has reacted with the bromine
53
Q

Addition reactions

A

A chemical reaction when a double bond is broken in an alkene resulting in the addition of atoms to the molecule - one product forms

54
Q

Hydrogenation

A

An addition reaction with an unsaturated compound and hydrogen to make a saturated compound - happens at 200˚C with a nickel catalyst

55
Q

Ethanol addition reaction

A

Ethene reacted with steam at 300˚C with phosphoric acid as a catalyst - H bonds with a carbon and -OH with another carbon

56
Q

Product of ethene reacting with bromine

A

Dibromoethane

57
Q

Two processes used to make ethanol

A
  • Fermentation - Glucose –> ethanol + carbon dioxide - enzymes in yeast break the glucose down in absence of air at 25-35˚C
  • Catalytic addition of steam to ethene - Ethene + Water –> Ethanol at 300˚C and 6000 kPa = 60 atmospheres & phosphoric acid as a catalyst
58
Q

Properties of ethanol

A
  • Liquid at room temp
  • Volatile
  • Boiling point of 78˚C
  • Highly flammable - blue flame with oxygen
  • Releases a lot of heat energy
  • Ethanol + Oxygen –> Carbon dioxide + Water
  • Substances can dissolve in ethanol - can be used as a solvent
  • Contains alkyl part
59
Q

Uses of ethanol

A
  • Cosmetics & perfumes - can dissolve substances water can’t
  • Perfume - High volatility leads to easy evaporation and diffusion
  • Fuel - combustion is highly exothermic & can be used as biofuel from crops
  • Hand sanitizers - microorganisms can’t survive in ethanol
60
Q

Pros and cons of fermentation’s sustainability

A
  • Pro - Fermentation uses crops and waste plant material which is sustainable
  • Con - Use of crops for fermentation can impact food supply
61
Q

Pros and cons of hydration’s sustainability

A
  • Con - Hydration uses petroleum from fossil fuels, which will eventually run out
62
Q

Pros and cons of fermentation’s process

A
  • Con - Fermentation requires ethanol to be produced in batches so it is a stop-start process
63
Q

Pros and cons of hydration’s process

A
  • Pro - Hydration can produce ethanol continuously to meet market demands
64
Q

Pros and cons of fermentation’s cost

A
  • Pro - Fermentation can be conducted at low temperatures so it is relatively inexpensive
65
Q

Pros and cons of hydration’s cost

A
  • Pro - Hydration can produce ethanol in a fully automated factory requiring little human input
  • Con - Hydration requires high temperatures and pressure, which is expensive
66
Q

Pros and cons of fermentation’s product

A
  • Con - Fermentation requires the impure product to be refined by fractional distillation
67
Q

Pros and cons of hydration’s product

A

Hydration can yield pure ethanol that does not need further refinement

68
Q

Most common carboxylic acid

A

Ethanoic acid - CH3COOH - dissolves in water to make a solution of pH 2.5

69
Q

Equation for an acid and metal reacting

A

Acid + Metal –> Salt + Hydrogen
e.g. Ethanoic acid + magnesium –> magnesium ethanoate + hydrogen

70
Q

Product of ethnic acids forming salts

A
  • Ethanoate ion - CH3COO^-
71
Q

Equation for an acid and base reacting

A

Acid + Base –> Salt + water
e.g. Ethanoic acid + Sodium hydroxide –> Sodium ethanoate + water

72
Q

Equation for an acid and carbonate reacting

A

Acid + Carbonate –> Salt + Water + Carbon dioxide
e.g. Ethanoic acid + Sodium carbonate –> Sodium ethanoate + water + carbon dioxide

73
Q

Two methods of oxidizing ethanol to get ethanoic acid

A
  • Acid fermentation - Using bacteria such as acetobacter with enzymes that catalyze the oxidation of ethanol to ethanoic acid and water
  • Using acidified potassium manganate(VII) - KMnO4 is a used as a strong oxidizing agent in the presence of sulfuric acid and heat to make ethanoic acid
74
Q

Properties and uses of esters

A
  • Homologous series
  • Used in modern consumer products
  • Fragrant - used in flavoring in food and cosmetic products
75
Q

Esterification

A

The process of producing and ester by reacting a carboxylic acid and an alcohol in the presence of an acid catalyst
e.g. Ethanol + Ethanoic acid –> Ethyl ethanoate + Water

76
Q

Describing how ethanol & ethanoic acid make an ester

A
  1. C-O bond of the OH hydroxyl group in ethanoic acid breaks
  2. The O-H bond in ethanol breaks
  3. the two remaining parts from each molecule join together forming a C-O bond for the ester
  4. OH and H combine to form water (condensation reaction)
77
Q

Naming an ester

A
  • First names comes from the alcohol
  • Second name comes from the carboxylic acid
78
Q

Polymerization reactions

A

When smaller molecules known as monomers build up to form a polymer molecule

79
Q

Common plastic

A

Polythene / poly (ethene)

80
Q

Making polythene

A
  • Addition polymerization
  • Very many ethene molecules react together joining end to end to make polytene molecules
81
Q

Repeat units

A
  • Used to draw the displayed formula of a whole molecule
  • Drawn inside brackets with a n to show a very large number of molecules to form the polymer
  • Change C=C bond to C-C and draw a line between then and draw brackets around the repeat unit & add n in writing a chemical equation
82
Q

Condensation reaction

A

When two smaller molecules join to produce a larger molecule - large and smaller molecule are produced (usually water is the smaller)

83
Q

Poor methods of plastic disposal

A
  • Land fills - Leachate can contaminate the surrounding area and nearby bodies of water
  • Burning - Incineration leads to toxic gases forming e.g. PVC releases acidic hydrogen chloride
84
Q

Polyamides

A
  • Condensation polymers
  • Made from a dicarboxylic acid containing two COOH groups & a diamine that contains two NH2 groups
  • Shown as block diagrams
  • O-H and H break of to make H2O
85
Q

Polyesters

A
  • Condensation polymers
  • Made of a dicarboxylic acid & a diol containing two OH groups
  • O-H and H break off to make H2O
  • Shown as block diagrams
86
Q

Amide link

A

A chemical bond in a polyamide with a C=O bond and an N-H bond

87
Q

Ester link

A

A chemical bond in polyester comprising of a C=O bond and a C-O bond

88
Q

Common polyester

A

PET

89
Q

Functional groups of amino acids

A
  • NH2 group
  • COOH group
90
Q

Meaning of R in an amino acid structure

A

Represents a side group that is specific to the amino acid e.g. hydrogen for glycine

91
Q

Occurrences in making an amino acid

A
  • COOH & NH2 group make an amide link
  • Molecule of water is eliminated

Chemistry IGCSE (12 decks)

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